What is the effect of increasing pressure on the dissociation of $PCl_5$ according to the equation $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)} - x \ cal$?

For the following reaction,which change will shift the equilibrium towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}; \Delta H_r^o(298 \ K) = +150 \ kJ$

In the production of $NO$,the reaction is $N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$,$\Delta H = +ve$. This reaction is favored by:

When a catalyst is added to a system,the:

The yield of product in the reaction,$A_{2(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$ would be higher at

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction is favored at constant temperature by: $(1)$ Adding an inert gas at constant volume $(2)$ Adding $Cl_{2(g)}$ at constant volume $(3)$ Adding an inert gas at constant pressure $(4)$ Increasing the volume of the container $(5)$ Adding $PCl_{5(g)}$ at constant volume